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chap-3

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 
The law of conservation of mass follows from the concept that
a.
atoms are indivisible.
b.
atoms of different elements have different properties.
c.
matter is composed of atoms.
d.
atoms can be destroyed in chemical reactions.
 

 2. 
The composition of the two oxides of lead, PbO and PbO2, are explained by the
a.
periodic law.
c.
atomic law.
b.
law of multiple proportions.
d.
law of conservation of mass.
 

 3. 
Who first proposed an atomic theory based on scientific knowledge?
a.
John Dalton
c.
Robert Brown
b.
Jons Berzelius
d.
Dmitri Mendeleev
 

 4. 
According to Dalton’s atomic theory, atoms
a.
are destroyed in chemical reactions.
b.
can be divided.
c.
of each element are identical in size, mass, and other properties.
d.
of different elements cannot combine.
 

 5. 
Which of the following is NOT part of Dalton’s atomic theory?
a.
Atoms cannot be divided, created, or destroyed.
b.
The number of protons in an atom is its atomic number.
c.
In chemical reactions, atoms are combined, separated, or rearranged.
d.
All matter is composed of extremely small particles called atoms.
 

 6. 
The law of definite proportions
a.
contradicted Dalton’s atomic theory.
b.
was explained by Dalton’s atomic theory.
c.
replaced the law of conservation of mass.
d.
assumes that atoms of all elements are identical.
 

 7. 
In a cathode tube, electrical current passes from one electrode, the _____, to the oppositely charged electrode.
a.
cathode
c.
negatively charged electrode
b.
anode
d.
Both (a) and (c)
 

 8. 
Experiments with cathode rays led to the discovery of the
a.
proton.
c.
neutron.
b.
nucleus.
d.
electron.
 

 9. 
Who explained the behavior of positively charged particles being deflected from a metal foil as the nucleus?
a.
Ernest Rutherford
c.
James Chadwick
b.
John Dalton
d.
Niels Bohr
 

 10. 
In the gold foil experiment, most of the particles fired at the foil
a.
bounced back.
c.
were absorbed by the foil.
b.
passed through the foil.
d.
combined with the foil.
 

 11. 
The gold foil experiment led to the discovery of the
a.
electron.
c.
nucleus.
b.
cathode ray.
d.
neutron.
 

 12. 
What did Rutherford conclude about the structure of the atom?
a.
An atom is indivisible.
b.
Electrons make up the center of an atom.
c.
An atom carries a positive charge.
d.
An atom contains a small, dense, positively charged central region.
 

 13. 
A nuclear particle that has about the same mass as a proton, but with no electrical charge, is called a(n)
a.
nuclide.
c.
electron.
b.
neutron.
d.
isotope.
 

 14. 
Which part of an atom has a mass approximately equal to chap-3-web_files/i0150000.jpg of the mass of a common hydrogen atom?
a.
nucleus
c.
proton
b.
electron
d.
electron cloud
 

 15. 
The mass of a neutron is
a.
about the same as that of a proton.
c.
double that of a proton.
b.
about the same as that of an electron.
d.
double that of an electron.
 

 16. 
The nucleus of most atoms is composed of
a.
tightly packed protons.
b.
tightly packed neutrons.
c.
tightly packed protons and neutrons.
d.
loosely connected protons and electrons.
 

 17. 
Protons and neutrons strongly attract when they
a.
are moving fast.
c.
are at high energies.
b.
are very close together.
d.
have opposite charges.
 

 18. 
An aluminum isotope consists of 13 protons, 13 electrons, and 14 neutrons. Its mass number is
a.
13.
c.
27.
b.
14.
d.
40.
 

 19. 
Isotopes are atoms of the same element that have different
a.
principal chemical properties.
c.
numbers of protons.
b.
masses.
d.
numbers of electrons.
 

 20. 
Atoms of the same element that have different masses are called
a.
moles.
c.
nuclides.
b.
isotopes.
d.
neutrons.
 

 21. 
Isotopes of an element contain different numbers of
a.
electrons.
c.
neutrons.
b.
protons.
d.
nuclides.
 

 22. 
When the light from excited atoms of an element is passed through a prism, the distinct colored lines produced are called
a.
ground states.
c.
line-emission spectra.
b.
excited states.
d.
electromagnetic spectra.
 

 23. 
Bohr’s theory helped explain why
a.
electrons have negative charge.
b.
most of the mass of the atom is in the nucleus.
c.
excited hydrogen gas gives off certain colors of light.
d.
atoms combine to form molecules.
 

 24. 
According to Bohr’s theory, an excited atom would
a.
collapse.
c.
produce line-emission spectra.
b.
absorb photons.
d.
radiate energy.
 

 25. 
If electrons in an atom have the lowest possible energies, the electrons are in their
a.
ground states.
c.
excited states.
b.
inert states.
d.
radiation-emitting states.
 

 26. 
For an electron in an atom to change from the ground state to an excited state,
a.
energy must be released.
b.
energy must be absorbed.
c.
radiation must be emitted.
d.
the electron must make a transition from a higher to a lower energy level.
 

 27. 
Most of the volume of an atom is occupied by the
a.
nucleus.
c.
electron cloud.
b.
nuclides.
d.
protons.
 

 28. 
The main energy levels of an atom are indicated by the
a.
orbital quantum numbers.
c.
spin quantum numbers.
b.
magnetic quantum numbers.
d.
principal quantum numbers.
 

 29. 
The letter designations for the first four sublevels, with the number of electrons that can be accommodated in each sublevel are
a.
s: 1, p: 3, d: 10, and f: 14.
c.
s: 2, p: 6, d: 10, and f: 14.
b.
s: 1, p: 3, d: 5, and f: 7.
d.
s: 1, p: 2, d: 3, and f: 4.
 

 30. 
The number of orbitals for the d sublevel is
a.
1.
c.
5.
b.
3.
d.
7.
 

 31. 
The statement that an electron occupies the lowest available energy orbital is
a.
Hund’s rule.
c.
Bohr’s law.
b.
the aufbau principle.
d.
the Pauli exclusion principle.
 

 32. 
“Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin” is a statement of
a.
the Pauli exclusion principle.
c.
the quantum effect.
b.
the aufbau principle.
d.
Hund’s rule.
 

 33. 
The statement that no more than two electrons in the same atom can occupy a single orbital is
a.
the Pauli exclusion principle.
c.
Bohr’s law.
b.
Hund’s rule.
d.
the aufbau principle.
 

 34. 
Which of the following rules requires that each of the p orbitals at a particular energy level receive one electron before any of them can have two electrons?
a.
Hund’s rule
c.
the aufbau principle
b.
the Pauli exclusion principle
d.
the quantum rule
 

 35. 
Two electrons in the 1s orbital must have different spin quantum numbers to satisfy
a.
Hund’s rule.
c.
the Pauli exclusion principle.
b.
the magnetic rule.
d.
the aufbau principle.
 

 36. 
The sequence in which energy sublevels are filled is specified by
a.
the Pauli exclusion principle.
c.
Lyman’s series.
b.
the orbital rule.
d.
aufbau principle.
 

 37. 
Which is the ground-state electron configuration for chap-3-web_files/i0380000.jpg?
a.
[Ar] 4s23d4
c.
[Ar] 4s33d3
b.
[Ar] 4s13d5
d.
[Ar] 4s43d2
 

 38. 
The carbon-12 atom is assigned a relative mass of exactly
a.
1 amu.
c.
12 amu.
b.
6 amu.
d.
100 amu.
 

 39. 
The abbreviation for atomic mass unit is
a.
amu.
c.
a.
b.
mu.
d.
µ.
 

Completion
Complete each sentence or statement.
 

 40. 
The statement that a chemical compound always contains the same elements in exactly the same proportions is called the law of _________________________.
 

 

 41. 
The statement that mass cannot be created or destroyed in ordinary chemical and physical changes is called the law of _________________________.
 

 

 42. 
The statement that when two elements combine to form two or more compounds, the mass of one element that combines with a given mass of the other element is in the ratio of small whole numbers is known as the law of _________________________.
 

 

 43. 
A subatomic particle that has a negative electric change is a(n) ____________________.
 

 

 44. 
An atom’s central region, which is made up of protons and neutrons, is the ____________________.
 

 

 45. 
A subatomic particle that has a positive charge and that is found in the nucleus of an atom is a(n) ____________________.
 

 

 46. 
A subatomic particle that has no charge and is found in the nucleus is a(n) ____________________.
 

 

 47. 
The number of protons in the nucleus of an atom is called the ____________________.
 

 

 48. 
The sum of the numbers of protons and neutrons of the nucleus of an atom is called the ____________________.
 

 

 49. 
An atom that has the same number of protons as other atoms of the same element but has a different number of neutrons is called a(n) ____________________.
 

 

 50. 
Another method of writing the nickel isotope, chap-3-web_files/i0520000.jpg, is ____________________.
 

 

 51. 
A region in an atom where there is a high probability of finding electrons is called a(n) ____________________.
 

 

 52. 
Orbitals are sometimes called electron ____________________ because they do not have hard boundaries.
 

 

 53. 
All of the frequencies or wavelengths of electromagnetic radiation make up the electromagnetic ____________________.
 

 

 54. 
The wavelength of electromagnetic radiation is inversely proportional to its ____________________.
 

 

 55. 
Light can be thought of as a stream of particles, the ____________________ of which is determined by the light’s frequency.
 

 

 56. 
A state in which an atom has more energy than it does in its ground state is called a(n) ____________________.
 

 

 57. 
A number that specifies a property of an orbital is called a(n) _________________________.
 

 

 58. 
The statement that two particles of a certain class cannot be in the exact same energy state is known as the ____________________ principle.
 

 

 59. 
The _________________________ of an atom is the arrangement of its electrons.
 

 

 60. 
The statement that the structure of each successive element is obtained by adding one proton to the nucleus of the atom and one electron to the lowest-energy orbital that is available is known as the ____________________ principle.
 

 

 61. 
The statement that for an atom in the ground state, the number of unpaired electrons is the maximum possible and these unpaired electrons have the same spin is known as ____________________ rule.
 

 

 62. 
The mass of an atom expressed in atomic mass units is the ____________________.
 

 

 63. 
The SI base unit used to measure the amount of a substance whose number of particles is the same as the number of particles in 12 g of carbon-12 is called the ____________________.
 

 

 64. 
Avogadro’s number has a value (to three significant figures) of ____________________.
 

 

 65. 
The mass in grams of 1 mol of a substance is the substance’s ____________________.
 

 

Short Answer
 

 66. 
What is the atomic number of the atom chap-3-web_files/i0690000.jpg?
 

 67. 
What is the mass number of the atom chap-3-web_files/i0700000.jpg?
 

 68. 
How many electrons are in a neutral atom of chap-3-web_files/i0710000.jpg?
 

 69. 
How many protons are in an atom of chap-3-web_files/i0720000.jpg?
 

 70. 
How many neutrons are in an atom of chap-3-web_files/i0730000.jpg?
 

 71. 
What is the molar mass of tin, which has an atomic mass of 118.7 amu?
 

Problem
 

 72. 
What is the mass of 2.5 moles of carbon?
 

 73. 
How many moles of copper are present in 180.0 g Cu?
 

 74. 
The mass of 1 mol of gold atoms is 196.97 g. Find the mass of 1 atom of gold.
 

 75. 
How many atoms are in 0.12 mol of cadmium?
 

Essay
 

 76. 
Describe atomic mass.
 

 77. 
Describe the atomic mass unit.
 

 78. 
How are the atomic mass unit and the atomic mass related?
 



 
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